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First Order Reaction

What is the c...

Question

What is the cell entropy change (in J K") of the following cell
The EMF of the cell is found to be 0.045 V at 298 K and temperature coefficient is :
$3.4 \times 10^{- 4} V K^{- 1}$
(Given: $K_{a (C H_{3} C O O H)} = 10^{- 5} M)$

$P t (s) ∣ ∣ ∣ \begin{matrix} H_{2} (g) p = 1 a t m \end{matrix} ∣ ∣ ∣ \begin{matrix} C H_{3} C O O H, H C l 0.1 M \end{matrix} ∣ ∣ ∣ ∣ ∣ ∣ \begin{matrix} K C l (a q) 0.1 M \end{matrix} ∣ ∣ ∣ \begin{matrix} H g_{2} C l_{2} (s) \end{matrix} ∣ ∣ ∣ H g$

60

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65.2

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69.2

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63.5

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Solution

The correct option is B $65.2$
As we know,
$Δ S = n F {(\frac{d E_{c e l l}}{d T})}_{P} = 2 \times 96500 \times 3.4 \times 10^{- 4}$
$= 65.2 J K^{- 1}$

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Similar questions

P t (x) | H_{2} (g) | C H_{3} C O O H, H C l | | K C l (a q) | H g_{2} C l_{2} (s) | H g

3.4 \times 10^{- 4} V K^{- 1}

K_{a (C H_{3} C O O H)} = 10^{- 5} M

P t (s) | H_{2} (g, 1 a t m) | C H_{3} C O O H, H C l | | K C l (a q) | H g_{2} C l_{2} (s) | H g

0.0045 V

3.4 \times 10^{- 4} V K^{- 1}

A g | A g C l | | K C l (a q .) | H_{2} C l_{2} | H g

3.38 \times 10^{- 4} V K^{- 1}

P b (s) + {H g C l}_{2} (a q) ⟶ {P b C l}_{2} (a q) + H g (l)

{(\frac{d E}{d T})}_{p} = 1.5 * 10^{- 4} V / K

F e | F e^{2 +} (a q) | | C d^{2 +} (a q) | C d

- 1.25 \times 10^{- 4} V K^{- 1}

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